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physics
electricity and magnetism
Conceptual Physics 11th edition Paul G. Hewitt - Solutions
Why are interference colors more apparent for thin films than for thick films?
Will the light from two very close stars produce an interference pattern? Explain.
Polarized light is a part of nature, but polarized sound is not. Why?
Why do radio waves diffract around buildings, while light waves do not?
Why will an ideal Polaroid filter transmit 50% of incident nonpolarized light?
Why may an ideal Polaroid filter transmit anything from zero to 100% of incident polarized light?
What percentage of light is transmitted by two ideal Polaroids, one on top of the other with their polarization axes aligned? With their axes at right angles to each other?
How can you determine the polarization axis for a single sheet of Polaroid (especially if you're at the edge of a lake)?
Why do Polaroid sunglasses reduce glare, whereas non polarized sunglasses simply cut down the total amount of light reaching the eyes?
How can a single sheet of Polaroid film be used to show that the sky is partially polarized? (Interestingly enough, unlike humans, bees and many insects can discern polarized light and use this ability for navigation.)
Light will not pass through a pair of Polaroid sheets when they are aligned perpendicularly. However, if a third Polaroid is sandwiched between the two with its alignment halfway between the alignments of the other two (that is, with its axis making a 45° angle with each of the other two alignment
Why did practical holography have to await the advent of the laser?
Light illuminates two closely spaced thin slits and produces an interference pattern on a screen behind. For which color of light-yellow or green-will the distance between the fringes be greater?
What is the evidence for the claim that iron exists in the relatively cool outer layer of the Sun?
How might the Fraunhofer lines in the spectrum of sunlight that are due to absorption in the Sun's atmosphere be distinguished from those due to absorption by gases in Earth's atmosphere?
In what specific way does light from distant stars and galaxies tell astronomers that atoms throughout the universe have the same properties as those on Earth?
A blue-hot star is about twice as hot as a red-hot star. But the temperatures of the gases in advertising signs are about the same, whether they emit red or blue light. What is your explanation?
Which has the greatest energy-a photon of infrared light, of visible light, or of ultraviolet light?
Does atomic excitation occur in solids as well as in gases? How does the radiant energy from an incandescent solid differ from the radiant energy emitted by an excited gas?
A lamp filament is made of tungsten. Why do we get a continuous spectrum rather than a tungsten line spectrum when light horn an incandescent lamp is viewed with a spectroscope?
Have you ever watched a fire and noticed that the burning of various materials often produces flames of different colors? Why is this so?
Since an absorbing gas re-emits the light it absorbs, why are there dark lines in an absorption spectrum? That is, why doesn't the re-emitted light simply fill in the dark places?
If atoms of a substance absorb ultraviolet light and emit red light, what becomes of the "missing" energy?
(a) Light from an incandescent source is passed through sodium vapor and then examined with a spectroscope. What is the appearance of the spectrum? (b) The incandescent source is switched off and the sodium is heated until it glows. How does the spectrum of the glowing sodium compare with the
Your friend reasons that if ultraviolet light can activate the process of fluorescence, infrared light ought to also. Your friend looks to you for approval or disapproval of this idea. What is your position?
When ultraviolet light falls on certain dyes, visible light is emitted. Why does this not happen when infrared light falls on these dyes?
Why are fabrics that fluoresce when exposed to ultraviolet light so bright in sunlight?
When a certain material is illuminated with visible light, electrons jump horn lower to higher energy states in atoms of the material. When illuminated by ultraviolet light, atoms are ionized as some of them eject electrons. Why do the two kinds of illumination produce such different results?
To keep chickens warm in a chicken coop, why would a CFL be a poor choice compared with an incandescent bulb?
The first laser consisted of a red ruby rod activated by a photoflash tube that emitted green light. Why would a laser composed of a green crystal rod and a photoflash tube that emits red light not work?
In the operation of a helium-neon laser, why is it important that the meta stable state in the helium atom closely match the energy level of a more-difficult-to-come-by meta stable state in neon?
A friend speculates that scientists in a certain country have developed a laser that produces far more energy than is put into it and asks for your response. What is your response?
Ultraviolet light causes sunburns, whereas visible light, even of greater intensity, does not. Why is this so?
We know that an incandescent lamp filament at 2500 K radiates white light. Does the lamp filament also radiate energy when it is at room temperature?
Since every object has some temperature, every object radiates energy. Why, then, can't we see objects in the dark?
If we continue heating a piece of initially room-temperature metal in a dark room, it will begin to glow visibly. What will be its first visible color, and why?
We can heat a piece of metal to red-hot and then to white-hot. Can we heat it until the metal glows blue-hot?
If you see a red-hot star, you can be certain that its peak intensity is in the infrared region. Why is this?
If you see a "violet-hot" star, you can be certain its peak intensity is in the ultraviolet range. Why is this?
If we double the frequency of light, we double the energy of each of its photons. If we instead double the wavelength of light, what happens to the photon energy?
We perceive a "green-hot" star not as green but as white. Why?
Sketch (a) below shows a radiation curve of an incandescent solid and its spectral pattern as produced with a spectroscope. Sketch (b) shows the "radiation curve" of an excited gas and its emission spectral pattern. Sketch (c) shows the curve produced when a cool gas is between an incandescent
Consider just four of the energy levels in a certain atom, as shown in the diagram. How many spectral lines will result from all possible transitions among these levels? Which transition corresponds to the highest-frequency light emitted? To the lowest-frequency light emitted?
For the transitions described in the previous exercise, is there any relationship among the wavelengths of the emitted photons?Previous exerciseAn electron de-excites from the fourth quantum level in the diagram of Exercise 52 to the third and then directly to the ground state. Two photons are
Suppose the four energy levels in Exercise 52 were somehow evenly spaced. How many spectral lines would result?
If light were passed through a round hole instead of a thin slit in a spectroscope, how would the spectral "lines" appear? What is the drawback of a hole in comparison with a slit?
If we use a prism or a diffraction grating to compare the red light from a common neon tube and the red light from a helium-neon laser, what striking difference do we see?
In the diagram, the energy difference between states A and B is twice the energy difference between states B and C. In a transition (quantum jump) from C to B, an electron emits a photon of wavelength 600 nm.a. What is the wavelength emitted when the photon jumps from B to A?b. When it jumps from C
What does it mean to say that something is quantized?
Silver bromide (AgBr) is a light-sensitive substance used in some types of photographic film. To cause exposure of the film, it must be illuminated with light having sufficient energy to break apart the molecules. Why do you suppose this film may be handled without exposure in a darkroom
Sunburn produces cell damage in the skin. Why is ultraviolet radiation capable of producing this damage, while visible radiation, even if more intense, is not?
In the photoelectric effect, does brightness or frequency determine the kinetic energy of the ejected electrons? Which determines the number of the ejected electrons?
A very bright source of red light has much more energy than a dim source of blue light, but the red light has no effect in ejecting electrons from a certain photosensitive surface. Why is this so?
Why does light striking a metal surface eject only electrons, not protons?
Explain how the photoelectric effect is used to open automatic doors when someone approaches.
Explain briefly how the photoelectric effect is used in the operation of at least two of the following: an electric eye, a photographer's light meter, the sound track of a pre-digital motion picture.
Distinguish between classical physics and quantum physics.
If you shine an ultraviolet light on the metal ball of a negatively charged electroscope (shown in Exercises 11 and 12 in Chapter 22), it will discharge. But if the electroscope is positively charged, it won't discharge. Can you venture an explanation?
Discuss how the reading of the meter in Figure 31.1 will vary as the photosensitive plate is illuminated by light of various colors at a given intensity and by light of various intensities of a given color.
Does the photoelectric effect prove that light is made of particles? Do interference experiments prove that light is composed of waves? (Is there a distinction between what something is and how it behaves?)
Does Einstein's explanation of the photoelectric effect invalidate Young's explanation of the double-slit experiment? Explain.
The camera that took the photograph of the woman's face (Figure 31.4) used ordinary lenses that are well known to refract waves. Yet the step-by-step formation of the image is evidence of photons. How can this be? What is your explanation?
Light has been argued to be a wave and then a particle, and then back again. Does this indicate that light's true nature probably lies somewhere between these two models?
In the previous chapter, we learned the formula E ~ f. In this chapter, we learned the formula E = hf. Explain the difference between these two formulas. What is h?
If a cannonball and a BB have the same speed, which has the longer wavelength?
We don't notice the wavelength of moving matter in our common experience. Is this because the wavelength is extraordinarily large or extraordinarily small?
What principal advantage does an electron microscope have over an optical microscope?
Would a beam of protons in a "proton microscope" exhibit greater or less diffraction than electrons of the same speed in an electron microscope? Defend your answer.
Comment on the idea that the theory one accepts determines the meaning of one's observations and not vice versa.
A friend says, "If an electron is not a particle, then it must be a wave." What is your response? (Do you hear "either-or" statements like this often?)
Consider one of the many electrons on the tip of your nose. If somebody looks at it, will its motion be altered? How about if it is viewed with one eye closed? With two eyes open, but crossed? Does Heisenberg's uncertainty principle apply here?
Do we inadvertently alter the realities that we attempt to measure in a public opinion survey? Does Heisenberg's uncertainty principle apply here?
If the behavior of a system is measured exactly for some period of time and is understood, does it follow that the future behavior of that system can be exactly predicted? (Is there a distinction between properties that are measurable and properties that are predictable?)
II a butterfly causes a tornado, does it make sense to eradicate butterflies? Defend your answer.
To measure the exact age of Old Methuselah, the oldest living tree in the world, a Nevada professor of dendrology, aided by an employee of the U.S. Bureau of Land Management, cut the tree down in 1965 and counted its rings. Is this an extreme example of altering that which you measure or an example
We speak of photons of red light and photons of green light. Can we speak of photons of white light? Why or why not?
A typical wavelength of infrared radiation emitted by your body is 25 mm (2.5 × 10-2 m). Show that the energy per photon of such radiation is about 8.0 × 10-24 J.
Consider the de Broglie wavelength of an electron that strikes the back face of one of the early models of a TV screen at 1/10 the speed of light. Show that the electron wavelength is 2.4 × 10-11 m.
You decide to roll a 0.1-kg ball across the floor so slowly that it will have a small momentum and a large de Broglie wavelength. If you roll it at 0.001 m/s, what is its wavelength? How does this compare with the de Broglie wavelength of the high-speed electron in the previous problem?
Figure 32.10 shows three transitions among three energy levels that would produce three spectral lines in a spectroscope. If the energy spacing between the levels were equal, would this affect the number of spectral lines?
How can elements with low atomic numbers have so many spectral lines?
How does the wave model of electrons orbiting the nucleus account for discrete energy values rather than a continuous range of energy values?
Why do helium and lithium exhibit very different chemical behavior, even though they differ by only one electron?
The Ritz combination principle can be considered to be a statement of energy conservation. Explain.
Why does no stable electron orbit with a circumference of 2.5 de Broglie wavelengths exist in any atom?
Can a particle be diffracted? Can it exhibit interference?
How does the amplitude of a matter wave relate to probability?
If Planck's constant, h, were larger, would atoms be larger also? Defend your answer.
If the world of the atom is so uncertain and subject to the laws of probabilities, how can we accurately measure such things as light intensity, electric current, and temperature?
When we say that electrons have particle properties and then continue to say that electrons have wave properties, aren't we contradicting ourselves? Explain.
When and where do Newton's laws of motion and quantum mechanics overlap?
In what way did Rutherford's gold-foil scattering experiment show that the atomic nucleus is both small and very massive?
Does the correspondence principle have application to macroscopic events in the everyday macro world?
Richard Feynman, in his book The Character of Physical Law, states: "A philosopher once said, 'It is necessary for the very existence of science that the same conditions always produce the same results.' Well, they don't!" Who was speaking of classical physics, and who was speaking of quantum
What does the wave nature of matter have to do with the fact that we can't walk through solid walls, as Hollywood movies often show using special effects?
Largeness or smallness has meaning only relative to something else. Why do we usually call the speed of light "large" and Planck's constant "small"?
How does Rutherford's model of the atom account for the back-scattering of alpha particles directed at the gold foil?
Why does classical physics predict that atoms should collapse?
Which type of radiation-alpha, beta, or gamma-produces the least change in mass number? In atomic number?
In bombarding atomic nuclei with proton "bullets," why must the protons be accelerated to high energies if they are to make contact with the target nuclei?
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